Chapter 7

A sample of \(12.7\) grams of sodium sulfate (Na2SO4) is dissolved in \(672 \mathrm{~mL}\) of distilled water. a. What is the molar concentration of sodium sulfate in the solution? b. What is the concentration of sodium ion in the solution?

1\. A 1.50 mL aliquot of a \(0.177 \mathrm{M}\) solution of sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) is diluted into \(10.0 \mathrm{~mL}\) of distilled water, to give solution A. A \(10.0 \mathrm{~mL}\) aliquot of \(\mathbf{A}\) is then diluted into \(50.0 \mathrm{~mL}\) of distilled water, to give solution \(\mathbf{B}\). Finally, \(10.0 \mathrm{~mL}\) of \(\mathbf{B}\) is diluted into \(900.0 \mathrm{~mL}\) of distilled water to give solution C. Additional distilled water is then added to \(\mathrm{C}\) to give a final volume of \(1.0000 \mathrm{~L}\). What is the final concentration of sulfuric acid in solution C? 2\. A solution was prepared by mixing \(250 \mathrm{~mL}\) of \(0.547 \mathrm{M} \mathrm{NaOH}\) with \(50.0 \mathrm{~mL}\) of \(1.62 \mathrm{M} \mathrm{NaOH}\) and then diluting to a final volume of \(1.50 \mathrm{~L}\). What is the molarity of \(\mathrm{Na}^{+}\) in this solution? To what final volume should \(75.00 \mathrm{~mL}\) of \(0.889\) M HCl(aq) be diluted to prepare \(0.800 \mathrm{M} \mathrm{HCl}(\mathrm{aq})\) ?

For each of the molecules of \(\mathrm{NH}_{3}\) and \(\mathrm{CO}_{2}\) indicate whether a molecular dipole exists. If a dipole does exist, use a dipole arrow to indicate the direction of the molecular dipole.

Calculate the mass of sodium chloride required to make \(125.0 \mathrm{~mL}\) of a \(0.470 \mathrm{M} \mathrm{NaCl}\) solution. If you dissolve \(5.8 \mathrm{~g}\) of \(\mathrm{NaCl}\) in water and then dilute to a total of \(100.0 \mathrm{~mL}\), what will be the molar concentration of the resulting sodium chloride solution?